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Understanding Factors Affecting Reaction Rates in Chemistry

In this video, we explore the key factors that influence reaction rates, including temperature, reactant concentration, catalysts, and the nature of reactants. We discuss the difference between homogeneous and heterogeneous reactions, how to identify them, and why homogeneous reactions tend to be faster. Practical examples, including the combustion of iron and various chemical reactions, illustrate these principles. By the end, viewers will understand how to increase the rate of reactions through various methods, backed by solid examples and explanations.

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Understanding Factors Affecting Reaction Rates in Chemistry

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  1. Factors affecting rxn rates #3

  2. http://www.youtube.com/watch?v=5tFy9bOLsxw Iron Combustion!

  3. Increasing the Rate of Reactions 1. Increasing temperature 2. Increasing reactant concentration 3. Adding a catalyst(aninhibitor decreases) triggers a reaction rate to increase; participates in the reactions but comes out the same way it went in. 4. Nature of the reactant(changing a reactant for a more reactive one) • Increasing the pressure • Increasing the surface area – only for heterogeneous rxns!

  4. Homogeneous Vs Heterogeneous Reactions A homogeneous reaction is one where all the reactants are in the samephase. They are fast due to thorough mixing and manycollisions! H2(g) + O2(g) → AgNO3(aq) + NaCl(aq) → same- only look at reactants!

  5. Factors that Affect the Reaction Rate Heterogeneousreactants are in two or more different phases Slow due to poor mixing and fewer collisions Zn(s) + 2HCl(aq) → Fe(s) + O2(g) →

  6. heterogeneous Classify as Homogeneous or Heterogeneous: 2.                   Ag+(aq)  +  Cl (aq)          →       AgCl  (s)                    homogeneous 1.  Zn (s)  +  2HCl (aq)       →       H2(g)  +  ZnCl2  (aq) homogeneous 3.                   H2(g)    +  F2(g)        →              2HF (g)                                     

  7. What reactions are faster? ( in general ) 1. Homo’s are fasterthan hetero’s. 2. FastestSlowest (aq) (g and l) (s) only reactants 3. Simple ionicare fastest -no bonds to break- double replacement AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) Becomes: Ag+ + NO3- + Na+ + Cl- → AgCl(s) + Na+ + NO3- Fast Ag+ + Cl- → AgCl(s) Fast simple ionic!

  8. Describe each Pair of reactions as faster or slower. 2NaClO3(aq) + F2(aq) → 2NaF(aq) + 3O2(g) + Cl2(g) Faster Homo 3H2(g) + N2(g)  2NH3(g) Homos are fast- more collisions Aqueous reactions are fasters than gaseous. Homo

  9. Describe each Pair of reactions as faster or slower. Zn(s) + 2HCl(aq)  H2(g) + ZnCl2(aq)  Faster because aq ions: 1. close proximity in soln 2. ability to move through solvent 3. strong +/- interactions. Hetero C(s) + O2(g)  CO2(g) Hetero

  10. State five ways to increase the rate of this reaction. Mg(s) + 2HCl(aq) → H2(g) + MgCl2(aq) 1. Increase temperature 2. Increase [HCl], add more Mg 3. Add a catalyst 4. Increase surface area (powder Mg) 5. Agitate

  11. Hebden, p 7. Exercises 10 – 11; p 8. Exercises 12 – 14; p 9. Exercises 15 – 16 AND 17. (Read page12 on Collision Theory to fill in the blanks for tomorrow’s lecture)

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